Achemist designs a galvanic cell that uses these two half-reactions: Answers the

Question

Achemist designs a galvanic cell that uses these two half-reactions:

Answers the following question about this cell.

a) write a balance equation fo the half-reactionthat happens at the cathode.

b) write a balanced equation for the half-reaction atthe anode.

c) wrrite a balance equation for the overall reaction thatpowers the cell. be sure the reaction is spontanous as written.

d) do you have enough information to calculate the cell voltage under standard conditions?

e) if you said it was possible to calculate the cell voltage, do so and enter your answer here. be sure your answer has the correct number of significant digits.

THIS IS ONE QUESTION. AND CAN U PLEASE SHOW CALCULATION . AND SOLVE ASAP

half-reaction Standard reduction potential 2H2o(l)+2e->h2(g)+2oh-(aq) E^0red=-0.83V Zn^2+(aq)+2e-->zn(s) E^0red=0.673V

Explanation / Answer

a) Zn+2(aq) + 2e- -----> Zn(s)

b) H2(g) + 2OH- (aq) -----> 2H2O(l) + 2e-

c) Zn+2 + H2 + 2OH- ------> Zn + 2H2O

d) yes

e) at standard conditions P=1atm and concentrations are 1M so:

E= E0 - RT/nF LnQ = (0.673 - (-0.83)) - 8.314x 273/2 x 96500 Ln 1

E= 1.503 V

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